Textbook Question
The ΔH°f of TiI3(s) is –328 kJ/mol and the ΔH ° for the reaction 2 Ti(s) + 3 I2(g) → 2 TiI3(s) is –839 kJ. Calculate the ΔH of sublimation of I2(s), which is a solid at 25 °C.
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Ch.6 - Thermochemistry
Chapter 6, Problem 117
A copper cube with an edge measuring 1.55 cm and an aluminum cube with an edge measuring 1.62 cm are both heated to 55.0 °C and submerged in 100.0 mL of water at 22.2 °C. What is the final temperature of the water when equilibrium is reached? (Assume a density of 0.998 g/mL for water.)
Verified step by step guidance1
Calculate the volume of each cube using the formula for the volume of a cube: \( V = a^3 \), where \( a \) is the edge length.
Determine the mass of each cube using the formula \( m = \rho \times V \), where \( \rho \) is the density of the material. Use the densities: copper (8.96 g/cm³) and aluminum (2.70 g/cm³).
Calculate the heat lost by each metal cube using the formula \( q = m \times c \times \Delta T \), where \( c \) is the specific heat capacity (copper: 0.385 J/g°C, aluminum: 0.897 J/g°C) and \( \Delta T \) is the change in temperature.
Calculate the heat gained by the water using the formula \( q = m \times c \times \Delta T \), where \( m \) is the mass of the water (100.0 mL \( \times \) 0.998 g/mL), \( c \) is the specific heat capacity of water (4.18 J/g°C), and \( \Delta T \) is the change in temperature.
Set the heat lost by the metal cubes equal to the heat gained by the water and solve for the final temperature \( T_f \) when equilibrium is reached.
Related Practice
Textbook Question
A gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and the rest propane (C3H8) by volume. When the fuel mixture contained in a 1.55 L tank, stored at 755 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion is in the gaseous state.)
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Textbook Question
A gaseous fuel mixture stored at 745 mmHg and 298 K contains only methane (CH4) and propane (C3H8). When 11.7 L of this fuel mixture is burned, it produces 769 kJ of heat. What is the mole fraction of methane in the mixture? (Assume that the water produced by the combustion is in the gaseous state.)
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Open Question
A pure gold ring and a pure silver ring have a total mass of 14.9 g. The two rings are heated to 62.0 °C and dropped into 15.0 mL of water at 23.5 °C. When equilibrium is reached, the temperature of the water is 25.0 °C. What is the mass of each ring? (Assume a density of 0.998 g/mL for water.)